If the water temperature in your experiment was measured as 23.8degrees C and th

Question

If the water temperature in your experiment was measured as 23.8degrees C and the barometric pressure was given as 753 mmhg, what volumn of h2(g) would you expect to produce if you reacted .38 g of calcium metal with excess hcl? If you weighted out 0.38 g os calcium and reacted it with an excess amount of HCl how many moles of H2(g) would you expect to produce? 3. If the water temperature in your experiment was measured as 23.8 degree C and the barometric pressure was given as 753 mmHg, what volume of H2(g) would you expect to produce if you reacted 0.38g of calcium metal with excess HCl?

Explanation / Answer

Ca + 2HCl --------> CaCl2 + H2

0.38 g Ca * 1 mole Ca * 1 moles H2

1     40 g Ca 1 mole Ca

= 0.0095 moles of H2 = "n"

P = 753 mm Hg * (1 atm / 760 mm Hg) = 0.990 atm

T = 23.8 degrees C = 23.8 + 273.15 = 296.95 K

R = 0.0821 L-atm / mole * K

V = ?

PV = nRT

V = nRT / P

= 0.0095 * 0.0821 * 296.95

0.990

V = 0.2339 L

0.38 is 2 significant figures, so volume = 0.23 litres

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